Honors Chem Semester 1 Final Review

What are the diatomic atoms?

What are the diatomic atoms?

Hydrogen, Oxygen, Nitrogen, and Halogens (HON Halogens)

Quantative measurement

Involves a number

Qualitative measurement

Relates to quality instead of a number

What are the different types of matter?

Gas, liquid, and solid

What are the steps to the scientific method?

1)make observations

2)formulate hypotheses

3)perform experiments

Physical property

Characteristics that are directly observable and unique to a substance (ex. Odor, color, volume, state, density, or melting/boiling point)

Physical change

Changes in 1 or more physical properties of a substance, not in its chemical composition

Chemical property

A substance's ability to form new substances; describe the behavior of matter (ex. Flammability, the rusting of steel, digestion of food, etc.)

Chemical change

A change in the identify of a substance

Solid characteristics

Organized, close together, fixed volume and shape

Liquid characteristics

Less organized, semi-close, definite volume, and takes the shape of its container

Gas characteristics

Unorganized, moving quickly, no definite volume or shape

Metals

Left side of the periodic table, except hydrogen

Properties of metals

Good at conducting heat and electricity, malleable, ductile (able to be drawn out into thin wire), and has a lustrous and shiny appearance

Metalloids

Elements that have some metal and nonmetal properties

Metalloid properties

Have a combination of metallic and nonmetallic properties, most are very reactive, not usually found in combined forms (ex. Noble metals-gold, platinum, and silver)

Nonmetals

Appear on the right side of the periodic table

Nonmetal properties

Lack properties of metals, have a variety of properties, and can be gases, solids, or liquids

Group 1

Alkali metals

Group 2

Alkali-earth metals

Group (1)7

Halogens

Group (1)8

Noble gases

Group 3-12

Transition metals

What are the subatomic particles?

Electron, neutron, and proton

Proton

Positive 1 charge and mass of 1836

Electron

Negative charge of 1 and mass of 1

Neutron

Neutral charge and mass of 1839

Dalton

Created Dalton's atomic theory (1.Elements are made of tiny particles called atoms; 2.All atoms of a given element are identical; 3. The atoms of a given element are different from those of any other element; 4. Atoms of one element can combine with atoms of other elements to form compounds. A given compound always has the same relative numbers and types of atoms; 5. Atoms are indivisible in chemical processes. That is, atoms are not created or destroyed in chemical reactions. A chemical reaction simply changes the way the atoms are grouped together.)

Thomson

Founded electrons

Kelvin

Created the plum pudding model(idea that the atom might be something like plum pudding—a pudding with raisins randomly distributed throughout. The atom might be thought of as a uniform "pudding" of positive charge with enough negative electrons scattered within to counterbalance that positive charge.)

Mendeleev

Arranged the elements and essentially created the periodic table.

Rutherford

Created the Rutherford model that proved Kelvin's plum pudding model wrong

Arrhenius

Arrhenius proposed that an acid is a substance that produces H+ ions when it is dissolved in water. Arrhenius also found that aqueous solutions that exhibit basic behavior always contain hydroxide ions. He defined a base as a substance that produces hydroxide ions in water.

Binary compound

A compound made of 2 elements

Ionic compound

Metal with a nonmetal

Covalent compound

Nonmetal with nonmetal

Type 1

Metal forms only one cation(groups 1-3, zinc, and silver); ends in -ide

Type 2

Metal can form 2 or more cations(transition metals); uses Roman numerals to indicate charge on the metal cation (I ATE acid and it was IC-ky and O US we ITE)

Type 3

Uses prefixes

Precipitation reaction

Double displacement and a solid forms

Acid-base reaction

Product includes water and reactants include hydrogen(H) and hydroxide(OH)

What are the different types of oxidation-reduction reactions?

Formation of a gas/single-replacement reaction, combustion reaction, synthesis reaction, and decomposition reaction

Formation of gas

Single replacement (A+BC->B+AC)

Combustion reaction

Involves oxygen and produces energy in the form of heat

Synthesis reaction

Compound becomes simpler (A+B->AB)

Decomposition reaction

Compound is broken down into simpler substances (AB->A+B)

Mega(M)

1,000,000

Kilo(k)

1,000

Deci(d)

0.1

Centi(c)

0.01

Milli(m)

0.001

Micro(weird u looking symbol)

0.000001

Nano(n)

0.000000001

Celsius to kelvin formula

Temperature in kelvin=temperature in Celsius+273

Kelvin to Celsius formula

Temperature in Celsius=temperature in kelvin-273

Fahrenheit to Celsius formula

Temperature in Celsius=(temperature in Fahrenheit-32)/1.80

Celsius to Fahrenheit formula

Temperature in Fahrenheit=1.80(temperature in Celsius)+32

Mono-

1

Di-

2

Tri-

3

Tetra-

4

Penta-

5

Hexa-

6

Hepta-

7

Octa-

8